2. Which one of the following statements is incorrect? (a) According to the Gibbs phase rule, four phases of a pure substance cannot exist (b) All triple points correspond to a gas-liquid-solid equilibrium (c) The triple point in a P-T diagram becomes a triple line in a P-V diagram (d) The chemical potential determines which of several phases is the most stable

2. Which one of the following statements is incorrect? (a) According to the Gibbs phase rule, four phases of a pure substance cannot exist (b) All triple points correspond to a gas-liquid-solid equilibrium (c) The triple point in a P-T diagram becomes a triple line in a P-V diagram (d) The chemical potential determines which of several phases is the most stable

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 16Q: Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is...

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What mass (g) of ethanol, CH3CH2OH(), can be vaporized at its boiling point of 78.4 C by transfer of 500. kJ to the liquid? The vapH of ethanol is 38.6 kJ/mol at this temperature.
Which one of the following statements is incorrect? (a) According to the Gibbs phase rule, four phases of a pure substance cannot exist (b) All triple points correspond to a gas-liquid-solid equilibrium (c) The triple point in a P-T diagram becomes a triple line in a P-V diagram (d) The chemical potential determines which of several phases is the most stable
The phase diagram of a hypothetical substance is (a) Estimate the normal boiling point and freezing point ofthe substance. (b) What is the physical state of the substanceunder the following conditions? (i) T = 150 K, P = 0.2 atm;(ii) T = 100 K, P = 0.8 atm; (iii) T = 300 K, P = 1.0 atm.(c) What is the triple point of the substance?
Suppose you have two colorless molecular liquids, one boilingat -84 °C, the other at 34 °C, and both at atmosphericpressure. Which of the following statements is correct? Foreach statement that is not correct, modify the statement sothat it is correct. (a) The higher-boiling liquid has greatertotal intermolecular forces than the lower-boiling liquid. (b)The lower-boiling liquid must consist of nonpolar molecules.(c) The lower-boiling liquid has a lower molecular weightthan the higher-boiling liquid. (d) The two liquids have identicalvapor pressures at their normal boiling points. (e) At-84 °C both liquids have vapor pressures of 760 mm Hg.
(3) Vapor pressure of liquid ethanol is 7291 Pa at 20°C. (a) one student reports that the vapor pressure is 31741 Pa at 52°C. Another student reports it to be 31741 Pa at 502°C. Which of the results is correct? Why? (b) calculate the normal boiling temperature of ethanol (assume Patm=101,325Pa).
Elemental carbon has one gas phase, one liquid phase, and two different solid phases, as shown in the phase diagram: (a) On the phase diagram, label the gas and liquid regions.(b) Graphite is the most stable phase of carbon at normal conditions. On the phase diagram, label the graphite phase.(c) If graphite at normal conditions is heated to 2500 K while the pressure is increased to 1010 Pa, it is converted into diamond. Label the diamond phase.(d) Circle each triple point on the phase diagram.(e) In what phase does carbon exist at 5000 K and 108 Pa?(f) If the temperature of a sample of carbon increases from 3000 K to 5000 K at a constant pressure of 106 Pa, which phase transition occurs, if any?
A 5.4-L closed vessel is filled with 0.46 g of liquid ethanol. This ethanol containing closed vessel is placed in the freezer and reaches the vapor pressure of 6.65 torr at -11 C. (i) Is there any liquid ethanol remained in the closed vessel when the container is removed and warmed to the temperature of 25 C? Justify your answer. (ii) How many grams of liquid ethanol remained in the vessel at 2.0 C? The enthalpy changes of vaporization, AH,vap of ethanol is 40.5 kJ/mol. The molar mass of ethanol is 46.07 g/mol.
Liquid butane (C4H10) is stored in cylinders to be used as afuel. The normal boiling point of butane is listed as -0.5 °C.(a) Suppose the tank is standing in the sun and reaches atemperature of 35 °C. Would you expect the pressure in thetank to be greater or less than atmospheric pressure? Howdoes the pressure within the tank depend on how muchliquid butane is in it? (b) Suppose the valve to the tank isopened and a few liters of butane are allowed to escape rapidly.What do you expect would happen to the temperatureof the remaining liquid butane in the tank? Explain.(c) How much heat must be added to vaporize 250 g ofbutane if its heat of vaporization is 21.3 kJ/mol? What volumedoes this much butane occupy at 755 torr and 35 °C?
If heat is added to ice and liquid water in a closed container, and after the addition of heat there is still ice and liquid water remaining. (a)the vapor pressure of water will decrease. (b)the temperature will increase some. (c)the temperature will decrease some. (d)the vapor pressure of water will rise. (e)the vapor pressure of water will remain constant
The phase diagram for elemental sulfur is shown in Figure 6.18. (a) How many allotropes are shown? (b) What is the stable allotrope of sulfur under normal conditions of temperature and pressure? (c) Describe the changes to sulfur as its temperature is increased from 25?C while at 1 atm pressure.
Consider the phase diagram shown below: (a) Identify the different phases that occur in each region of the phase diagram. What is the value of the normal melting point and the normal boiling point for the compound? Identify the triple point and the critical point on the phase diagram. (b) If the dashed line at 1 atm of pressure is followed from 100 to 500 °C, what phase changes will occur (in order of increasing temperature)? (c) What phase changes will occur if the pressure is decreased to 0.100 atm?
Sulfur exhibits two solid phases, rhombic and monoclinic. Use the accompanying phase diagram for sulfur given below to answer the questions that follow. (A). How many triple points are in the phase diagram? (B). What phases are in equilibrium at the topmost triple point? (C). How many phase transitions are there when rhombic sulfur at 1 atm and 80°C is heated to 500°C at constant pressure?